Acids and Bases

Buffers and Buffer Solutions MCQs with Answers

Welcome to the Buffers and Buffer Solutions MCQs with Answers, it helps learners quickly identify areas for improvement in Buffers and Buffer Solutions Online Test.

Buffers are essential in chemistry and biology for maintaining stable pH levels in solutions, crucial for various biochemical and industrial processes. Buffer solutions consist of a weak acid and its conjugate base (or vice versa), which resist changes in pH upon addition of small amounts of acid or base.

In Buffers and Buffer Solutions, understanding their properties is key. MCQs on buffers and buffer solutions often cover topics such as identifying effective buffer components, calculating pH changes upon addition of acids or bases, and recognizing the importance of buffer capacity in maintaining pH stability.

Buffer capacity multiple choice questions assess the ability of a buffer to resist pH changes, influenced by the concentrations of the buffer components. Buffer preparation MCQs focus on the correct methods and concentrations required to prepare effective buffer solutions for specific pH ranges.

pH control exam questions delve into applications of buffers in scenarios requiring precise pH adjustment, such as in biological systems or chemical processes. Buffer systems MCQs explore different types of buffer systems, including biological buffers like the phosphate buffer system in cells or industrial buffers used in manufacturing processes.

Buffers and Buffer Solutions Online Quiz

By presenting 3 options to choose from, Buffers and Buffer Solutions Quiz which cover a wide range of topics and levels of difficulty, making them adaptable to various learning objectives and preferences. You will have to read all the given answers of Buffers and Buffer Solutions Questions and Answers and click over the correct answer.

  • Test Name: Buffers and Buffer Solutions MCQ Quiz Practice
  • Type: Quiz Test
  • Total Questions: 40
  • Total Marks: 40
  • Time: 40 minutes

Note: Answer of the questions will change randomly each time you start the test. Practice each quiz test at least 3 times if you want to secure High Marks. Once you are finished, click the View Results button. If any answer looks wrong to you in Quiz, simply click on question and comment below that question, so that we can update the answer in the quiz section.

Buffers and Buffer Solutions MCQs

Buffers and Buffer Solutions Quiz

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A buffer system can be destroyed by

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The addition of a strong acid to a buffer solution will result in

3 / 40

A buffer solution can be made by mixing

4 / 40

The addition of a strong base to a buffer solution will result in

5 / 40

When an acid is added to a buffer, it reacts with

6 / 40

The main role of a buffer is to

7 / 40

When a base is added to a buffer, it reacts with

8 / 40

A buffer is most effective when

9 / 40

The main component of the intracellular buffer system is

10 / 40

The buffering region of a buffer is typically

11 / 40

The presence of a buffer in a solution

12 / 40

The optimal pH range of a buffer is determined by

13 / 40

Blood is an example of a

14 / 40

The phosphate buffer system is important in

15 / 40

Buffers are made from

16 / 40

A buffer solution is less effective when

17 / 40

In the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]), [HA] represents

18 / 40

Buffers are essential in biochemical assays to

19 / 40

When a small amount of acid is added to a buffer solution, the pH

20 / 40

The pH of a buffer solution depends on

21 / 40

Buffer solutions are important in

22 / 40

The Henderson-Hasselbalch equation is used to

23 / 40

The buffering capacity is maximum when

24 / 40

A solution with equal concentrations of a weak acid and its conjugate base has a pH

25 / 40

When a small amount of base is added to a buffer solution, the pH

26 / 40

A weak acid and its conjugate base are found in

27 / 40

Buffers are crucial in maintaining the pH of

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A buffer with a higher concentration of acid and its conjugate base will have a

29 / 40

A common example of a buffer system is

30 / 40

The buffer capacity is

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To prepare a buffer solution of pH 7, you would choose an acid with a pKa of

32 / 40

Ammonium chloride and ammonia form a buffer system. Ammonia acts as

33 / 40

The bicarbonate buffer system in blood maintains a pH around

34 / 40

Which of the following can act as a buffer?

35 / 40

The pH of a buffer solution is 4.5. If the pKa of the acid is 4.5, then the ratio [A-]/[HA] is

36 / 40

The effectiveness of a buffer is reduced when

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The effectiveness of a buffer solution is known as

38 / 40

In the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]), [A-] represents

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A buffer solution

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Buffers can resist changes in pH when small amounts of

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Buffers and Buffer Solutions Flashcards

A buffer solution

resists changes in pH

Buffers are made from

a weak acid and its salt

The main role of a buffer is to

maintain pH stability

A common example of a buffer system is

acetic acid and sodium acetate

The pH of a buffer solution depends on

the ratio of acid to salt

The buffer capacity is

the amount of acid or base the buffer can neutralize

The Henderson-Hasselbalch equation is used to

calculate the pH of a buffer solution

In the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]), [A-] represents

the concentration of the conjugate base

In the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]), [HA] represents

the concentration of the acid

A buffer solution can be made by mixing

acetic acid and sodium acetate

The pH of a buffer solution is 4.5. If the pKa of the acid is 4.5, then the ratio [A-]/[HA] is

0.042361111111111

A buffer is most effective when

the concentrations of the acid and its conjugate base are equal

The buffering region of a buffer is typically

pH = pKa ± 1

Blood is an example of a

natural buffer system

The bicarbonate buffer system in blood maintains a pH around

7.4

A buffer with a higher concentration of acid and its conjugate base will have a

higher buffer capacity

To prepare a buffer solution of pH 7, you would choose an acid with a pKa of

around 7

When a small amount of acid is added to a buffer solution, the pH

remains relatively constant

When a small amount of base is added to a buffer solution, the pH

remains relatively constant

The phosphate buffer system is important in

maintaining the pH of intracellular fluids

Ammonium chloride and ammonia form a buffer system. Ammonia acts as

a weak base

The addition of a strong acid to a buffer solution will result in

a small change in pH

The addition of a strong base to a buffer solution will result in

a small change in pH

Buffer solutions are important in

chemical reactions and biological processes

A solution with equal concentrations of a weak acid and its conjugate base has a pH

equal to the pKa of the acid

A buffer solution is less effective when

the pH is far from the pKa of the acid

Which of the following can act as a buffer?

CH3COOH and CH3COONa

A buffer system can be destroyed by

adding too much strong acid or base

The main component of the intracellular buffer system is

phosphate ions

The effectiveness of a buffer is reduced when

diluted excessively

The buffering capacity is maximum when

pH = pKa

Buffers are crucial in maintaining the pH of

enzyme-catalyzed reactions

When an acid is added to a buffer, it reacts with

the conjugate base

When a base is added to a buffer, it reacts with

the weak acid

The presence of a buffer in a solution

minimizes pH changes

The optimal pH range of a buffer is determined by

the pKa of the acid

Buffers are essential in biochemical assays to

maintain a stable pH

A weak acid and its conjugate base are found in

buffer solutions

The effectiveness of a buffer solution is known as

buffer capacity

Buffers can resist changes in pH when small amounts of

strong acids or bases are added

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